It is to your advantage to do this, since you may obtain partial credit if you do and you will receive little or no credit if you do not. Attention should be paid to significant figures. 1. N2(g) + 3H2(g) 2 NH3(g) For the reaction represented above, the value of the equilibrium constant, K., is 3.1 x 104 at 700. K. (a) Write the expression for the equilibrium constant, K., for the reaction. Assume the initial partial pressures of the gases are as follows: (b) (i) =0.411 atm, =0.903 atm, and =0.224 atm. Calculate the value of the reaction quotient, Q, at these initial conditions. (ii) Predict the direction in which the reaction will proceed at 700. K if the initial partial pressures are those given above. Justify your answer. Calculate the value of the equilibrium constant, K, given that the value of K, for the reaction at 700. K is 3.1 x 10-4. The value of K, for the reaction represented below is 8.3 x 103 at 700. K. P (c) (d) (i) NH4HS(g) (NH3(g) + H2S(g) (ii) 2 HS(g) +N2(g) + 3H2(g) ( 2 NH HS(g) NH3(g) + H2S(g) (NH HS(g) Calculate the value of K, at 700. K for each of the reactions represented below.